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Atomic / Electronic Structure

Stoichiometry and Moles

Aqueous Chemistry

Gases and Enthalpy

Structure and Bonding

100

A pair of isotopes has:

(A) the same number of protons and a different number of neutrons.

(B) the same number of protons and neutrons but a different number of electrons.

(D) the same number of neutrons and the same number of electrons.

(A) the same number of protons and a different number of neutrons.

100

Avogadro's number equals the number of:
(A) atoms in one mole of 0₂.

(B) atoms in one mole of atoms.

(D) atoms in one mole of atoms and marbles in one mole of marbles.

100

What is the strongest electrolyte in dilute aqueous solution?

(A) HClO₄
(B) HCN
(C) HF
(D) HNO₂

(A) HClO₄

100

A negative delta H values for a reaction implies that it is:

(A) Endothermic
(B) Exothermic
(C) Spontaneous
(D) Can not be determined

(B) Exothermic

100

Which molecule contains carbon with a negative formal charge?

(A) CO
(B) CO₂
(C) H₂CO
(D) CH₄

(A) CO

200

Which atom has the most neutrons?

(A) neon-20

(B) chlorine-35

(B) phosphorous-32

(D) sulfur-35

200

Which sample contains the least number of atoms?

(A) 1.00g C
(B) 1.00g O₂
(C) 1.00g H₂
(D) 1.00g Fe

(D) 1.00g Fe

200

What is/are the spectator ion(s) in this reaction?
HC₂H₃O₂(aq) + NaOH(aq) -> NaC₂H₃O₂(aq) + H₂O(l)

(A) C₂H₃O₂^- only

(B) H⁺ and OH^-

(D) Na⁺ and C₂H₃O₂^-

200

All gases approach ideal behavior under conditions of:

(A) low density and high temperature.
(B) low density and low temperature.
(C) high density and high temperature.
(D) high density and low temperature.

(A) low density and high temperature.

200

Which molecule has a 120° bond angle?

(A) CO₂
(B) NH₃
(C) IF₃
(D) SO₃

(D) SO₃

300

Alkaline earth metals form:

(A) +1 ions.
(B) +2 ions.
(C) +3 ions.
(D) -1 ions.

(B) +2 ions.

300

What mass of carbon is present in 0.500 mol of sucrose - C₁₂H₂₂0₁₁ (342 g/mol)?

(A) 6.01 g
(B) 72.0 g
(C) 144.g
(D) 288. g

(B) 72.0 g

300

What is the molar concentration of the chloride ion in a 3.0 M CaCl₂ solution?

(A) 6.0M
(B) 3.0M
(C) 1.5M
(D) 1.0M

(A) 6.0M

300

A 14.0 g sample of N₂ (g) occupies what volume at 0 C and 1.00 atm?

(A) 5.60 L

(B) 11.2 L

300

Which molecule is polar?
(A) CCl₄
(B) CS₂
(C) PH₃
(D) PF₅

400

Which atom has the largest atomic radius?

(A) K

(B) I

(D) Sn

400

Ibuprofen, a common pain reliever, contains 75.7% carbon, 15.5% oxygen, and 8.80% hydrogen by mass. What is the empirical formula?

(A) C₆H₉O
(B) C₉HO₂
(C) C₁₃H₁₈O₂
(D) C₇₆H₉O₁₆

400

What is the oxidation number of Mo in MoO₄^2-?

(A) +2
(B) +4
(C) +6
(D) +8

400

A 10.0 L sample of an ideal gas at 25.0 C is heated at constant pressure until the volume has doubled. What is the final temperature of the gas?

(A) 50.0 C
(B) 149 C
(C) 323 C
(D) 596 C

400

How many valence electrons are in the carbonate ion, CO₃^2-?

(A) 20
(B) 22
(C) 24
(D) 32

500

Which species has this ground-state electron arrangement? 1s²2s² 2p⁶3s² 3p⁶3d¹⁰

(A) Ni

(B) Ni²⁺

(D) Zn²⁺

500

How many moles of iron are necessary to react completely with 1.75 mol of oxygen gas?
30₂(g) + 4Fe(s)---> 2Fe0₃(s)

(A) 1.31 mol
(B) 1.75 mol
(C) 2.33 mol
(D) 5.25 mol

500

What mass (in g) of magnesium nitrate, Mg(NO₃)₂, are required to produce 250.0 mL of a 0.0750 M solution?

(A) 0.0188 g
(B) 0.0445 g
(C) 1.61 g
(D) 2.79 g

(D) 2.79 g

500

A 10.0 g sample of silver is heated to 100.0 °C and then added to 20.0 g of water (4.184 J/g*°C) at 23.0 °C in an insulated calorimeter. At thermal equilibrium, the temperature if the system was measured as 25.0 °C. What is the specific heat of silver?

(A) 0.053 J/g*°C
(B) 0.22 J/g*°C
(C) 4.5 J/g*°C
(D) 8.4 J/g*°C

(B) 0.22 J/g*°C

500

The best Lewis structure of N₂H₂ shows:

(A) a nitrogen-nitrogen triple bond.

(B) a nitrogen-nitrogen single bond.

(D) each nitrogen with two non-bonding electron pairs.